The principal quantum number, n, describes the energy level of a particular orbital as a function of the distance from the center of the nucleus. Additional quantum numbers exist to quantify the other characteristics of the electron. The angular momentum quantum number (§¤), the magnetic quantum number (m§¤), and the spin quantum number (ms) have strict rules which govern the possible values. Identify allowable combinations of quantum numbers for an electron. Select all that apply.

Here are the rules.
n can be any whole number over zero; i.e., 1, 2, 3, 4, etc.

l ("ell") can be any whole number beginning with zero, 1, 2, 3, etc with a maximum of n-1.

ml = - ell to + ell in whole numbers;i.e., if ell is 2 then ml can be -2,-1,0,+1,+2.

ms may have two values only; i.e., +1/2 or -1/2
Your job is to take these rules and apply them to each of the above and find those that are allowed. To give you a fast start
#1 is allowed.
#2 is not allowed. Why not? If N is 4, then l CAN be 2 (l can have values in this case of 0,1,2,3) so 2 is allowed. However, ml CANNOT be 3 because ml may take values from -l to +l (in whole numbers) which will allow -2,-1,0,+1,and +2 but not +3.